Chapter 11 Notes
Christina Park
2/14/12 pd.3
Chapter 11 Notes
I. Measuring Matter
A. Counting Particles number of unit for counting is always constant.
a. What is a mole? mole (mol): the SI unit used to measure the amount of a substance, number of representative particles. representative particle: any kind of particle such as atoms, molecules, formula units, electrons, or ions. Avogadro's number: 6.022 136 7 x 10²³, volume of one mole of a gas determined by Amedeo Avagadro in 1811.
B. Converting Moles to Particles and Partciles to Moles number of moles x 6.02 x 10²³ representative particles /1 mole = number of representative particles number of representative particles x 1 mole / 6.02 x 10²³ representative particles = number of moles
II. Mass and the Mole
A. The Mass of a Mole each atom of carbon-12 has a mass of 12 atomic mass units (amu). atomic masses of all other elements are established relative to carbon-12 molar mass: the mass in grams of any pure substance. molar mass of any element is numerically equal to its atomic mass and has the units g/mol.
B. Using Molar Mass number of moles x number of grams / 1 mole = mass
III. Moles of Compounds
A. Chemical Formulas and the Mole the chemical formula for a compound indicates the type of atoms and the number of each contained in one unit of the compound.
B. The Molar Mass of Compounds the mass of a mole of a compound equals the sum of the masses of every particle that makes up the compound. number of moles x molar mass = number of grams molar mass of a compound demonstrates the law of conservation of mass.
C. Converting Mole of a Compound to Mass calculate molar mass of compound. convert mol to g by using the molar mass as a conversion factor. moles x number of grams / 1 mole = mass
D. Converting the Mass of a Compound to Moles calculate molar mass of compound. use inverse of the molar mass as the conversion factor. mass x 1 mole
2/14/12 pd.3
Chapter 11 Notes
I. Measuring Matter
A. Counting Particles number of unit for counting is always constant.
a. What is a mole? mole (mol): the SI unit used to measure the amount of a substance, number of representative particles. representative particle: any kind of particle such as atoms, molecules, formula units, electrons, or ions. Avogadro's number: 6.022 136 7 x 10²³, volume of one mole of a gas determined by Amedeo Avagadro in 1811.
B. Converting Moles to Particles and Partciles to Moles number of moles x 6.02 x 10²³ representative particles /1 mole = number of representative particles number of representative particles x 1 mole / 6.02 x 10²³ representative particles = number of moles
II. Mass and the Mole
A. The Mass of a Mole each atom of carbon-12 has a mass of 12 atomic mass units (amu). atomic masses of all other elements are established relative to carbon-12 molar mass: the mass in grams of any pure substance. molar mass of any element is numerically equal to its atomic mass and has the units g/mol.
B. Using Molar Mass number of moles x number of grams / 1 mole = mass
III. Moles of Compounds
A. Chemical Formulas and the Mole the chemical formula for a compound indicates the type of atoms and the number of each contained in one unit of the compound.
B. The Molar Mass of Compounds the mass of a mole of a compound equals the sum of the masses of every particle that makes up the compound. number of moles x molar mass = number of grams molar mass of a compound demonstrates the law of conservation of mass.
C. Converting Mole of a Compound to Mass calculate molar mass of compound. convert mol to g by using the molar mass as a conversion factor. moles x number of grams / 1 mole = mass
D. Converting the Mass of a Compound to Moles calculate molar mass of compound. use inverse of the molar mass as the conversion factor. mass x 1 mole